Two intracellular molecules A and B, are normally synthesized at a constant rate of 1000 molecules per second per cell. The degradation rate of A is 0.01/s and B is 0.1/s

A}Write a differential equation to describe how the number of molecules of A and B change over time

B}What is the steady state value of A and B? How many molecules of A and B will there be after 1 second at steady state?

C}If the rate of synthesis of both A and B were suddenly increased 10-fold to 10,000 molecules per second—without any change in their degradation rate—how many molecules of A and B would there be after one second?

D}Which molecules would be preferred for responding rapidly changing environment? Explain your answer

How can electronegativity change themselves when in the Periodic System moving vertically down through a main group (for a higher atomic masses) and horizontally in the system (for a higher group numbers)

I need a second set of eyes!! Does this make sense?

Once glucose is placed in a baggie we placed in distilled water. We pulled a sample of water from the bottom of the beaker and added Benedict solution to it which turned it to a light blue. Adding Benedict solution to glucose tests for presence of reducing sugars that have the aldehyde functional group. – CHO. Once the Benedict solution turned glucose solution to light blue it was then heated in boiling distilled water. Positive results indicates a color change to orange proving diffusion occured. The bright red on the bottom of the tube indicates the presence of the aldehyde group. Benedict solution is a deep-blue alkaline solution because it contains copper sulfate. When mixed with glucose and heated, glucose oxidizes and gives up an electron that copper accepts and then become reduced which turns Benedict’s solution and sugar into an orange color and blue copper ion is reduced to a red copper ion. Therefore, because glucose can reduce copper in the Benedict Solution, it’s called a reducing sugar. Test was not redone. Our group and the group we compared our results with had same results and color.

Determine the pH of each of the following solutions.

Part A

0.24 M KCHO2

Express your answer to two decimal places.

Part B

0.22 M CH3NH3I

Express your answer to two decimal places.

Part C

0.21 M KI

Express your answer to two decimal places.

define and provide expamples for each of the following

1) qualitative photochemistry

2) quantitative photochemistry

What volumes (in mL) of 1.0 M triethanolamine and 1.0M HNO3 is required to prepare 1.0L of pH 7.76 buffer using triethanolamine that is 0.020 M in both triethanolamine and triethanolammonium ion?

4. Under each of the following conditions, please predict the effect the mutation will have on the rate at which glycolysis will proceed in liver cells:

a. Loss of the allosteric site for ATP in phosphofructokinase

b. Loss of binding site for citrate in phosphofructokinase

c. Loss of the phosphatase domain of the bifunctional enzyme that controls the level of fructose 2,6-bisphosphate

d. Loss of the binding site for fructose 1,6-bisphosphate in pyruvate kinase.

Consider the following equilibrium:
N2O4(g)?2NO2(g)
Thermodynamic data on these gases are given in Appendix C in the textbook. You may assume that ?H? and ?S? do not vary with temperature.

Part A At what temperature will an equilibrium mixture contain equal amounts of the two gases? Express your answer using four significant figures

Part B

At what temperature will an equilibrium mixture of 1 atm total pressure contain twice as much NO2 as N2O4?

Express your answer using four significant figures.

Part C

At what temperature will an equilibrium mixture of 9 atm total pressure contain twice as much NO2 as N2O4?

Express your answer using four significant figures.

Part D

Rationalize the results from parts B and C by using Le Chatelier's principle (Section 15.7 in the textbook).

Why do bubbles rise to the surface of Guinness slower than they rise to the surface of a light beer? (The beers are of very similar viscosity).If you poured the two beers very carefully into the same glass what would you expect to see?

In the balanced equilibrium reaction: 2 H2S <----> S2 + 2 H2, with K = 3.7 x 10-6, if the initial concentration of H2S is 0.080 M, what is the final concentration of H2?

How many grams of solute are in each of the following solutions?

0.437 L of a 0.350 M K2CO3 solution =

15.5 mL of a 2.50 M AgNO3 solution =

25.2 mL of a 6.00 M H3PO4 solution =

Calculate the pH for each of the following cases in the titration of 50.0 mL of 0.120 M HClO(aq) with 0.120 M KOH(aq). The ionization constant for HClO can be found here. (a) before addition of any KOH (b) after addition of 25.0 mL of KOH (c) after addition of 40.0 mL of KOH (d) after addition of 50.0 mL of KOH (e) after addition of 60.0 mL of KOH

A solution of HCl is prepared by diluting 25.0 mL of a 1.0 M HCl solution with enough water to make 750 mL of HCl solution. (Show your work for all calculations!)

a) What is the molarity of the HCl solution?

b) What is the [H3O+] and the pH of the HCl solution?

c) Write the balanced chemical equation for the reaction of HCl and Ba(OH)2

d) How many milliliters of the diluted HCl solution is required to completely react with 350 mg of Ba(OH)2?

What is the change in enthalpy (in kJ) under standard conditions when 33.75 g of lithium hydroxide dissolves in water? What is the change in enthalpy (in kJ) under standard conditions when 26.58 g of potassium hydroxide dissolves in water? What is the change in enthalpy (in kJ) under standard conditions when 181.37 g of sodium sulfate dissolves in water?

Find ΔE° for the reaction below if the process is carried out at a constant pressure of 1.00 atm andΔV (the volume change) = -24.5 L. (1 L ∙ atm = 101 J)
2 CO(g) + O₂ (g) → 2 CO₂(g) ΔH° = -566. kJ

Select one:

A. +2.47 kJ

B. -568 kJ

C. -2.47 kJ

D. -564 kJ